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Test of Academic Skills (TEAS)

General, Organic, and Biological Chemistry

Chemistry Topics Review

January, 2014

Dr. Ben Tovrog

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Periodic Table of the Elements

1H

1.008

2He

4.003

3Li

6.941

4Be

9.012

11Na

22.99

12Mg

24.31

19K

39.10

20Ca

40.08

37Rb

85.47

38Sr

87.62

55Cs

132.9

56Ba

137.3

87Fr

(223)

88Ra

(226)

21Sc

44.96

22Ti

47.88

39Y

88.91

40Zr

91.22

71Lu

175.0

72Hf

178.5

103Lr

(260)

104Rf

(261)

23V

50.94

24Cr

52.00

41Nb

92.91

42Mo

95.94

73Ta

180.9

74W

183.9

105Db

(262)

106Sg

(266)

25Mn

54.94

26Fe

55.85

43Tc

(98)

44Ru

101.1

75Re

186.2

76Os

190.2

107Bh

(262)

108Hs

(265)

27Co

58.93

45Rh

102.9

77Ir

192.2

109Mt

(266)

57La

138.9

58Ce

140.1

60Nd

144.2

61Pm

(145)

62Sm

150.4

63Eu

152.0

59Pr

140.9

89Ac

(227)

90Th

232.0

92U

238.0

93Np

(237)

94Pu

(242)

95Am

(243)

91Pa

(231)

28Ni

58.69

29Cu

63.55

46Pd

106.4

47Ag

107.9

78Pt

195.1

79Au

197.0

30Zn

65.39

48Cd

112.4

80Hg

200.6

64Gd

157.3

65Tb

158.9

67Ho

164.9

68Er

167.3

69Tm

168.9

70Yb

173.0

66Dy

162.5

96Cm

(247)

97Bk

(247)

99Es

(252)

100Fm

(257)

101Md

(258)

102No

(259)

98Cf

(251)

31Ga

69.72

32Ge

72.6149In

114.8

50Sn

118.7

81Tl

204.4

82Pb

207.2

33As

74.92

51Sb

121.8

83Bi

209.0

34Se

78.96

35Br

79.90

52Te

127.6

53I

126.9

84Po

(209)

85At

(210)

36Kr

83.80

54Xe

131.3

86Rn

(222)

5B

10.81

6C

12.01

13Al

26.98

14Si

28.09

7N

14.01

15P

30.97

8

16.00

9F

19.00

16S

32.07

17Cl

35.45

10Ne

20.18

18Ar

39.953

4

5

6

7

3B(3)

4B(4)

5B(5)

6B(6)

7B(7) (9) (10)

1B(11)

2B(12)

3A(13)

4A 5A(15)

6A(16)

7A(17)

8A(18)

2

1

6

7

(8)

1A(1)

2A(2)

8B

Lanthanides

Actinides

MAIN–GROUPELEMENTS

MAIN–GROUPELEMENTS

110 111 112

(269) (272) (277)

Metals (main-group)Metals (transition)Metals (inner transition)MetalloidsNonmetals

114

(285)

PE

RIO

D

TRANSITION ELEMENTS

INNER TRANSITION ELEMENTS

O

(14)

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Unit Conversion: 1151 Chap. 1

p. 88.

1. Is a 5 km run or a 5 mile run longer?

2. How many inches are in 12.75 centimeters?

p. 90

1. How many milligrams are in 5 grams.

2. If 1 kilogram is approximately 2.2 pounds, how many pounds are there in 6 kilograms.

3. 3 pounds = ____ ounces

4. 20 cups = _____ quarts.

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Unit Conversion: 1151 Chap. 1

p.88. #1. Is a 5 km run or a 5 mile run longer? 5 miles is longer5 km * (0.621 mile/km) = 3.11 mile.

2. How many inches are in 12.75 centimeters? 12.75 cm*(1 in / 2.54 cm) = 5.02 in.

3. How many milligrams are in 5 grams. 5000 mg5 g * ( 1000 mg / g) = 5000 mg

4. If 1 kilogram is approximately 2.2 pounds, how many pounds are there in 6 kilograms.

6 kg * (2.2 pound / kg) = 13.2 pounds

5. 3 pounds = 48 ounces (3 pounds * 16 ounce/pound = 48 ounces)

6. 20 cups = 5 quarts. (20 cups * 1 quart / 4 cups) = 5 quart

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Atomic Structure:1151 Chap. 3

p. 157.

1. Describe the construction of the atom.

Referring to the periodic table:

2. What is the atomic number of iron?

3. What is the atomic mass of iron?

4. How many protons does iron have?

5. How many neutrons does iron have?

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Atomic Structure:1151 Chap. 3

p. 157. 1. Describe the construction of the atom. The atom is made up of three main subatomic particles, neutrons,

protons and electrons. Neutrons and protons are in the nucleus, and electrons are located in orbitals a distance from the nucleus. which have different shapes and energies.

2. Referring to the periodic table, what is the atomic number of iron? Atomic number = 26. (also the number of protons).

3. What is the atomic mass of iron? The value in the periodic table is 55.845 amu (atomic mass units).

4. How many protons does iron have? 26

5. How many neutrons does iron have? The main isotope of iron has mass number 56. Neutrons = mass number – protons =

56-26 = 30.

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Isotopes – 1151 Chap. 3

p. 1581. How many protons would a positively charged isotope ion of O-18

have?

2. How many protons would a negatively charged isotope ion of C-14 have?

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Isotopes – 1151 Chap. 3

P. 1581. How many protons would a positively charged isotope ion of O-18

have? Oxygen has atomic number 8, which means 8 protons. The charge on the ion does not affect the number of protons. (The charge on an ion results from changes in the number of electrons)

2. How many protons would a negatively charged isotope ion of C-14 have? Carbon has atomic number 6, which means 6 protons. The charge on an ion does not affect the number of protons.

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Effects of Catalysts – 1151 Chap. 9

p. 159. 1. Given reactants X and Y, a catalyst C and product Z, order

the following steps in the general catalytic reaction process.

XYC CZCZ C + ZX + C XCY + XC XYC

2. How does a catalyst increase the rate of a chemical reaction?

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Effects of Catalysts – 1151 Chap. 9

p. 1591. Given reactants X and Y, a catalyst C and product Z, order the

following steps in the general catalytic reaction process. X + C XCY + XC XYCXYC CZCZ C + Z

2. How does a catalyst increase the rate of a chemical reaction. Catalysts lower the activation energy of a reaction which has the result of increasing the reaction rate.

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Periodic Trends: 1151 Chap. 3.

P. 161. 1. Complete the following sentence: Within a given family in the periodic table, atomic radii _________ while

electronegativity _________.

2. Which groups on the periodic table contain the most metalloids?

3. A student has two material samples. One is a metal (A) and the other is a nonmetal (B). The student is trying to determine which one is the metal. Which of the following could the student observe”? (Select all that apply)

a.. Sample A and B both conduct an electric current.b. Sample A cools rapidly when refrigerated but Sample B does not. c. Sample B heats very slowly when heat is applied, but sample A heats

very quickly.

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Periodic Trends: 1151 Chap. 3.

p. 161. 1. Complete the following sentence: Within a given family in the periodic table, atomic radii increases while

electronegativity decreases.

2. Which groups on the periodic table contain the most metalloids? (4A, 5A, 6A. Shown also as group 14, 15, 16.

3. A student has two material samples. One is a metal (A) and the other is a nonmetal (B). The student is trying to determine which one is the metal. Which of the following could the student observe”? (Select all that apply)

a. Sample A and B both conduct an electric current.b. Sample A cools rapidly when refrigerated but Sample B does not. c. Sample B heats very slowly when heat is applied, but sample A heats

very quickly. Metals have low values of specific heat. This means they cool and heat

quickly. Nonmetals cool and heat slowly. Answers b, and c apply.Metals conduct electric current but nonmetals do not. Answer

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Enzymes as Catalysts - 1152

p. 162. Identify whether the following are TRUE or FALSE. 1. Enzymes participate in a limited number of chemical reactions

throughout the human body.

2. Enzymes act to lower the activation energy of chemical reactions.

3. An enzyme can reshape itself when placed in contact with a substrate.

4. The amino-acid structure of an enzyme is important to its function.

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Enzymes as Catalysts - 1152

p. 162. Identify whether the following are TRUE or FALSE. 1. Enzymes participate in a limited number of chemical reactions

throughout the human body. False

2. Enzymes act to lower the activation energy of chemical reactions. True

3. An enzyme can reshape itself when placed in contact with a substrate. True

4. The amino-acid structure of an enzyme is important to its function. True

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pH and H+ Concentration 1151 Chap. 10

p. 164. 1. Suppose the activity (concentration) of hydrogen ions in a solution is 1

part per ten thousand. Find the pH value of the solution.

2. Complete the following sentence:

Regarding bases, a ______ number of hydrogen ions is associated with a a basic solution (as opposed to an acidic solution) and red litmus paper will turn ______ in the presence of a base.

3. What does a difference of one unit on the pH scale represent in terms of H+ concentration?

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pH and H+ Concentration 1151 Chap. 10

p. 164. 1. Suppose the activity (concentration) of hydrogen ions in a solution is 1

part per ten thousand. Find the pH value of the solution. Is this a basic or acidic solution? The H+ concentration is 0.0001M, which is 1 x 10-4. pH = - log (H+) = -log 1 x 10-4) = 4.0. The solution is acidic. (pH below 7 is acidic)

2. Complete the following sentence:

Regarding bases, a smaller number of hydrogen ions is associated with a a basic solution (as opposed to an acidic solution) and red litmus paper will turn blue In the presence of a base.

3. What does a difference of one unit on the pH scale represent in terms of H+ concentration? Since pH = - log H+, one unit on the pH scale equals a factor of 10 in concentration.

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Hydrocarbons 1152

p. 166.1. What is the name and formula of the common saturated

hydrocarbon that has four carbons.

2. What is the name and formula of the common saturated hydrocarbon that has five carbons.

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Hydrocarbons 1152

1. What is the name and formula of the common saturated hydrocarbon that has four carbons.

Butane C4H10

2. What is the name and formula of the common saturated hydrocarbon that has five carbons.

Pentane. C5H12

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13 | 21

C=C double bond Cn H2n - general formula unsaturated

- not "saturated" with maximum hydrogens - unsaturated fats have some double bonds (easier to digest)

note that cycloalkanes also are Cn H2n

Alkenes

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Lewis Dot Structures 1151 Chap. 5

p. 1671. Why does hydrogen gas exist as H2 and never just

as H? 2. Regarding the Lewis structure for sulfur (S), how

many unshared pairs of electrons will sulfur have in neutral covalent compounds.

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Lewis Dot Structures 1151 Chap. 5

p. 1671. Why does hydrogen gas exist as H2 and never just

as H? A Stable H atom will contain 2 electrons to fill its 1s

orbital. Joining 2 H atoms with a single bond satisfies that need.

2. Regarding the Lewis structure for sulfur (S), how many unshared pairs of electrons will sulfur have in neutral covalent compounds.

Neutral sulfur atoms in dot structures will have two lone pairs of electrons and two bonds to other atoms. (Such as H2S, SCl2)

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Reactions 1151 Chap. 6, 10

p. 1701. Balance the reaction.

Ca(OH)2 + HCl H2O + CaCl2

Identify whether the following statements are TRUE or FALSE.

2. pH neutralization is an important oxidation-reduction reaction.

3. Metabolism is an important oxidation reduction reaction.

4. Combustion is an important acid-base reaction.

5. Photosynthesis is an important acid-base reaction.

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Reactions 1151 Chap. 6, 10

p. 170. #1. Balance the reaction.

Ca(OH)2 + 2 HCl 2 H2O + CaCl2

Identify whether the following statements are TRUE or FALSE.

2. pH neutralization is an important oxidation-reduction reaction. False, it is an acid base reaction

3. Metabolism is an important oxidation reduction reaction. True

4. Combustion is an important acid-base reaction. False – It is an oxidation-reduction reaction.

5. Photosynthesis is an important acid-base reaction. False – It is an important oxidation-reduction reaction.

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Properties of Water 1151 Chap. 8,10.

p. 171. Identify whether the following statements are TRUE or FALSE.

1. Water serves as the standard for pH and has a value of 6.

2. The maximum density of water is 4 oC.

3. Water has the standard electronegative value on the periodic table.

4. The Kelvin temperature scale is based on water’s triple-point.

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Properties of Water 1151 Chap. 8,10.

. p. 171.

Identify whether the following statements are TRUE or FALSE.

1. Water serves as the standard for pH and has a value of 6. FALSE Water is the standard solvent for pH and has a value of 7.0.

2. The maximum density of water is 4 oC.

3. Water has the standard electronegative value on the periodic table. FALSE. Electronegativity values are given for elements, not compounds. Water is a compound so it does not have an electronegativity value.

4. The Kelvin temperature scale is based on water’s triple-point. Identify whether the following statements are TRUE or FALSE. TRUE – Water’s triple point is 273.15 K, which is the value used to add to

celsius temperature to determine Kelvin temperature.

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Energy and Matter 1151 Chap. 2

p. 172Suppose a phase transition occurs between a liquid and gas at -196 oC.

What is the Kelvin temperature?

Identify whether the following statements are TRUE or FALSE. A certain amount of a substance is in a solid state but it is then melted to

form a liquid, and finally vaporized to form a gas. The solid has a volume of 1.0 cubic centimeter, the liquid occupies 0.75 cubic centimeters, and the gas expanded to 10.0 cubic meters.

1. The liquid is more dense than the gas. 2. The liquid is less dense than the solid. 3. The solid is more dense than the gas. 4. The liquid has the highest density of the three forms.

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Energy and Matter 1151 Chap. 2

p. 172. Suppose a phase transition occurs between a liquid and gas at -196 oC.

What is the Kelvin temperature? Degree K = Degree Celsius + 273. For this case, Degree K = -196+273 = 77 K

Identify whether the following statements are TRUE or FALSE. A certain amount of a substance is in a solid state but it is then melted to

form a liquid, and finally vaporized to form a gas. The solid has a volume of 1.0 cubic centimeter, the liquid occupies 0.75 cubic centimeters, and the gas expanded to 10.0 cubic meters.

1. The liquid is more dense than the gas. True2. The liquid is less dense than the solid. False (Density =

mass/volume). The mass stays the same and the volume decreased, so density increased for the liquid relative to the solid.

3. The solid is more dense than the gas. True4. The liquid has the highest density of the three forms. True

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Evaporation, Vaporization, Condensation. 1151 Chap. 2

p. 173. Complete the sentence below. The heat of vaporization (latent heat) refers to the energy necessary (at

constant temperature) to cause a complete phase change from a ________to a _____________.

Suppose a substance A has a mass of M grams and a latent heat of L cal/g. If substance B has a mass three times that of substance A and a latent heat 1/6 of that of substance A, what will be the ratio of the heat of vaporization of A compared to B?

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Evaporation, Vaporization, Condensation. 1151 Chap. 2p. 173.

Complete the sentence below. The heat of vaporization (latent heat) refers to the energy necessary (at

constant temperature) to cause a complete phase change from a liquid to a vapor.

Suppose a substance A has a mass of M grams and a latent heat of L

cal/g. If substance B has a mass three times that of substance A and a latent heat 1/6 of that of substance A, what will be the ratio of the heat of vaporization of A compared to B?

Heat = mass x HV. Mass B = 3*Mass(A). HV(B) = 1/6 HV(A)Heat (A) = Mass(A)*HV(A). Heat (B) = Mass(B) *HV(B) = 3*Mass(A)* 1/6HV(A). Heat (B) = 0.5 * Heat(A)Heat (A) = 2 times Heat (B)